chem test 2

NH4+

Ammonium

OH-

Hydroxide

NO3-

Nitrate

N02

Nitrite

SO4^2-

Sulfate

SO3^ 2-

Sulfite

CO3^ 2-

Carbonate

PO4 ^3-

Phosphate

One

Mono-

Two

Di-

Three

Tri-

Four

Tetra-

Five

Penta-

Six

Hexa-

Seven

Hepta-

Eight

Octa-

Nine

Nona-

Ten

Deca-

Group 1 ions

+1

Group 2 ions

+2

Group 13 ions

+3

Group 15 ions

-3

Group 16 ions

-2

Group 17 ions

-1

Group 18 ions

Usually 0

Group 1 name

Alkali metals

Group 2 name

Alkaline earth metals

Groups 3-12 name

Transition metals

Group 18 name

Noble gases

Group 17 name

Halogens

Naming binary acids (hydrogen + nonmetal)

Hydro + nonmetal root + ic acid

Naming oxyacids (hydrogen or oxygen + elements)

Polyatomic ending (-ate, -ite) + acid ending (-ic acid, -ous ending)

Formal charge

FC = (valence e-) - (lone pair e-) - ½ (number bonded electrons)

Electron pair geometry

Counts bonds and lone pairs

Molecular geometry

Only counts arrangement of atoms

2 regions + no lone pairs

Linear (180 degrees)

3 regions + no lone pairs

Trigonal planar (120 degrees)

3 regions + 1 lone pair

Bent (less than 120 degrees)

4 regions + no lone pairs

Tetrahedral (109.5 degrees)

4 regions + 1 lone pair

Trigonal pyramidal (about 107 degrees)

4 regions + 2 lone pairs

Bent (about 104.5 degrees)

5 regions + no lone pairs

Trigonal bipyramidal (90, 120, 180 degrees)

5 regions + 1 lone pair

Seesaw (approx. 90, 120, 180 degrees)

5 regions + 3 lone pairs

T-shaped (approx. 90, 180 degrees)

5 regions + 3 lone pairs

Linear (180)

6 regions + no lone pair

Octahedral (90,180 degrees)

6 regions + 1 lone pair

Square pyramidal ( approx. 90, 180 degrees)

6 regions + 2 lone pairs

Square planar (90, 180 degrees)

Delta electronegativity of 0-0.4

Non polar covalent

Delta electronegativity of 0.5-1.7

Polar covalent

Delta electronegativity of more than 1.7

Ionic

Wan der waals forces

Attractive forces between atoms and molecules

IMFs

Attraction or repulsion force that acts between neighboring molecules or particals

Dispersion/london dispersion forces

Temporary - constant motion of electrons in molecules and atoms result instantaneous dipoles

Dipole - dipole attractions

Stronger than dispersion forces- adjacent molecules line up so that the partial negative pole of one molecule is as close as possible to the partial positive pole of another molecule

Hydrogen bonding

Strongest van der waal force- type of dipole - dipole attraction where a H covalent bonds to either N,F, or O

Sigma bonds

End - to - end overlap — occurs when orbitals of two atoms extend into the same region of space

Pi bonds

Side - by - side overlap — two parallel p orbitals overlap along their sides

2 electron domains

Sp — linear

3 electron domains

Sp² — Trigonal planar

4 electron domains

Sp³ — tetrahedral

5 electron domains

Sp³d — Trigonal bipyramidal

6 electron domains

Sp³d² — octahedral

6 regions + 3 lone pairs

T - shape (<90 degrees)

6 region + 4 lone pairs

Linear (180 degrees)